+18-01 Q3. Calculate the [H] (concentration of the H*) of a HCI solution when the pH=2.88 **Hint to solve Q3: antilog pH = -log[H] Molar mass HC1= 36.458 CH*]=9+iles (PH) 10-288 ↓ 1.318x10 n mol 13x10-3 ml g mol Density HCI-1.18 ml
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![pH -log[H*]
=
+18-01
Molar mass H3PO4-97.994-B
10-2.88
mol
Q3. Calculate the [H] (concentration of the H*) of a HCl solution when the pH=2.88
**Hint to solve Q3: antilog
pH = -log[H]
Molar mass HC1= 36.458
GH*]=artilag (PH)
1.318x10²13x10-³ m
Density H₂PO4-1.888
g
mol
ml
Density HCI-1.18 ml](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21c9e2c1-3922-4190-983a-755fc6e01f0b%2F6aecb197-dd6a-4f82-a8ef-8da22f548f69%2F4ka028_processed.jpeg&w=3840&q=75)
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